Determination of pH values over the temperature range –60°C for some operational reference standard solutins and values of the conventional residual liquid-junction potentials

Partial molar volumes of aluminium chloride, aluminium sulphate and aluminium nitrate in water-rich binary aqueous mixtures of tetrahydrofuran

“…Fresh triple distilled water was used as standard solvent for preparing binary THF + water mixture. The density of dioxane was found 1.02250 gcm -3 at 303.15 K, is in good agreement with literature value of THF density value 12 (d = 1.02230 gm -3 ).…”

Consistency of pH standard values with the corresponding thermodynamic acid dissociation constants (Technical Report)

“…The pa, values thus obtained are conventionally adopted as reference values pa, = pH(S) (7) All measured pH(X) values depend on the material chosen for reference solution [6,7], as a result of (i) the validity of the Bates-Guggenheim convention for each standard solution through other models of electrolyte solutions in order to recommend a broader and more realistic basis. pH(S) values are conventionally assigned to chosen reference buffer solutions which are variously referred to as RVS (potassium hydrogen phthalate), PS (NBSNIST reference buffers 2 < pH < 10) and S (other recommended buffer standards) [l].…”

Stability of a Ag/AgCl Reference Electrode Equipped with an Ionic Liquid Salt Bridge Composed of 1-Methyl-3-octylimidazolium Bis(trifluoromethanesulfonyl)-amide in Potentiometry of pH Standard Buffers

“…3 is ascribed to the variation of the LJP between the KCl solution (phase III) and each buffer (phase IV), and that of the PBP between the IL (phase V) and the buffer (phase IV). The variation of the LJP between the KCl solution and each buffer is known to be within 0.01 pH or 0.6 mV at 25 C. 12 The PBP between the IL (phase V) and the buffer (phase IV) is determined dominantly by the distribution potential by the partition of the cation and anion constituting the IL between the IL and an aqueous solution, when the ionic strength of the aqueous solution contacting with the IL is higher than 1 mmol dm -3 . 3 We therefore presume that the variation of E in cell (A) was caused by the distribution potential of the IL between the IL and a buffer solution.…”